Question 1

The ideal gas equation is expected to be valid at

Accepted Answer

A)  low temperature. 
B)  low pressure. 
C)  high pressure. 
D)  low temperature and low pressure. 
E)  low temperature and high pressure. 
A)  low temperature. 
B)  low pressure. 
C)  high pressure. 
D)  low temperature and low pressure. 
E)  low temperature and high pressure. B

Question 2

In this chapter, some important applications of high vacuum are discussed. Pressures of 1.0 x 10-9 atm can be routinely achieved in the laboratory. CO is a common contaminant at these low levels. How many molecules of CO would be present if it was the only contaminant in a 1.0 L container at a pressure of 1.0 x 10-9 atm and 298 K?

Accepted Answer

2.5 x 10¹³

Question 3

Consider the van der Waals "b" coefficient for He, O2 and CO2 increases because

Accepted Answer

A)  the number of different atoms increases. 
B)  the intermolecular forces acting between molecules increases. 
C)  the strength of chemical bonds increases. 
D)  the volume occupied by the molecules becomes more significant as the size of the molecule increases. 
E)  the mass of the molecules increases. 
A)  the number of different atoms increases. 
B)  the intermolecular forces acting between molecules increases. 
C)  the strength of chemical bonds increases. 
D)  the volume occupied by the molecules becomes more significant as the size of the molecule increases. 
E)  the mass of the molecules increases. D

Question 4

A hair spray bottle will explode if under 9 atm of internal pressure. If this bottle is originally under 5 atm of pressure at 25˚C and is placed to close to a campfire and raises to 48˚C, what will be the pressure inside the bottle now?

Accepted Answer

The answer of A hair spray bottle will explode if...

Question 5

If atmospheric pressure atop Mount Everest is about 250 mm Hg, what is the partial pressure of oxygen?

Accepted Answer

The answer of If atmospheric pressure atop Mount Everest is...

Question 6

A gas mixture containing oxygen, nitrogen, and helium; if the partial pressure and mole fraction of oxygen is 425 Torr and 0.46, respectively, and the partial pressure of helium is 74 Torr, what is the partial pressure (in bar) of nitrogen in the mixture?

Accepted Answer

Must use mole fracti

Question 7

Consider a sample of gas in a tank. Under which of the following conditions would you expect the least ideal behaviour?

Accepted Answer

A)  high temperature and high pressure 
B)  high temperature and low pressure 
C)  moderate temperature and pressure 
D)  low temperature and low pressure 
E)  low temperature and high pressure 
A)  high temperature and high pressure 
B)  high temperature and low pressure 
C)  moderate temperature and pressure 
D)  low temperature and low pressure 
E)  low temperature and high pressure

Question 8

If the relative humidity at 28°C is 58.3 %, what is the dew point?

Accepted Answer

The answer of If the relative humidity at 28°C is...

Question 9

The level of mercury on the sample side of a manometer is 56 mm below that of the atmospheric side. If the atmospheric pressure is 1.05 bar, what is the pressure of the gas sample (in bar)?

Accepted Answer

The answer of The level of mercury on the sample...

Question 10

A sample of gas is cooled to its vapourization temperature. What is true before the sample reaches equilibrium between the liquid and gaseous phases?

Accepted Answer

A)  More molecules are depositing than vapourizing. 
B)  More molecules are condensing than vapourizing. 
C)  More molecules are vapourizing than condensing. 
D)  No liquid is present. 
E)  The liquid molecules have more kinetic energy than the gas molecules. 
A)  More molecules are depositing than vapourizing. 
B)  More molecules are condensing than vapourizing. 
C)  More molecules are vapourizing than condensing. 
D)  No liquid is present. 
E)  The liquid molecules have more kinetic energy than the gas molecules.

Question 11

Consider the van der Waals "a" coefficient for He, O2 and C6H6 increases because

Accepted Answer

A)  the number of different atoms increases. 
B)  the intermolecular forces acting between molecules increase. 
C)  the strength of chemical bonds increases. 
D)  the volume occupied by the molecules becomes more significant as the size of the molecule increases. 
E)  the mass of the molecules increases. 
A)  the number of different atoms increases. 
B)  the intermolecular forces acting between molecules increase. 
C)  the strength of chemical bonds increases. 
D)  the volume occupied by the molecules becomes more significant as the size of the molecule increases. 
E)  the mass of the molecules increases.

Question 12

Consider the van der Waals equation:

Accepted Answer

A)  the van der Waals "a" term is proportional to molecular size and "b" is proportional to the magnitude of intermolecular forces. 
B)  the van der Waals "b" term is proportional to molecular size and "a" is proportional to the magnitude of intermolecular forces. 
C)  large molecules tend to have smaller values for both a and b. 
D)  the van der Waals equation describes successfully describes the behaviour of non-ideal gases. 
A)  the van der Waals "a" term is proportional to molecular size and "b" is proportional to the magnitude of intermolecular forces. 
B)  the van der Waals "b" term is proportional to molecular size and "a" is proportional to the magnitude of intermolecular forces. 
C)  large molecules tend to have smaller values for both a and b. 
D)  the van der Waals equation describes successfully describes the behaviour of non-ideal gases.

Question 13

Which will occupy a larger volume, 10 moles of H2 (g) or 10 moles of propane, C3H8 (g)?

Accepted Answer

A)  H2 (g) 
B)  C3H8 (g) 
C)  They will occupy the same volume. 
A)  H2 (g) 
B)  C3H8 (g) 
C)  They will occupy the same volume.

Question 14

Cooling the gas in a container lowers the pressure because

Accepted Answer

A)  there are less atoms in the container. 
B)  the potential energy increases in the container. 
C)  there are less collisions with the wall of the container. 
D)  the molecules' impact with the wall are less energetic. 
E)  the molecules slow down so both force and number of collisions with the walls is reduced. 
A)  there are less atoms in the container. 
B)  the potential energy increases in the container. 
C)  there are less collisions with the wall of the container. 
D)  the molecules' impact with the wall are less energetic. 
E)  the molecules slow down so both force and number of collisions with the walls is reduced.

Question 15

If the compressibility factor, pV/nRT is 1 at pressure p, then

Accepted Answer

A)  the gas is ideal. 
B)  the gas may be ideal, but is not necessarily ideal. 
C)  the gas is not ideal. 
D)  the gas is under optimum conditions. 
A)  the gas is ideal. 
B)  the gas may be ideal, but is not necessarily ideal. 
C)  the gas is not ideal. 
D)  the gas is under optimum conditions.

Question 16

Methylamine, whose line structure is shown below, is one of the substances for the "fishy" odour of not-so-fresh fish.   What is the average velocity and average kinetic energy (kJ/mole) of gaseous methylamine molecules at 25°C?

Accepted Answer

3.7 x 10³ k

Question 17

If 760 Torr is equivalent to 1 atm and to 1.01325 bar, then a pressure of 1 bar is equivalent to

Accepted Answer

A)  760 Torr. 
B)  770.07 Torr. 
C)  750.06 Torr. 
D)  129.86 Torr. 
E)  133.32 Torr. 
A)  760 Torr. 
B)  770.07 Torr. 
C)  750.06 Torr. 
D)  129.86 Torr. 
E)  133.32 Torr.

Question 18

A glass bulb with a volume of 250.0 mL contains a small amount of solid potassium chlorate. It is connected to a mercury manometer. Upon heating the bulb, the following (unbalanced) reaction occurs:
KClO3  $\rarr$  KCl + O2
After the apparatus cools back to room temperature, 23°C, the difference in the mercury levels in the manometer is now 14.2 cm. Which of the following statements are true?
1) The mercury on the side of the tube connected to the manometer is higher than before.
2) About 1.9 x 10-3 moles KClO3 decomposed.
3) About 0.16 g KClO3 decomposed.
4) The mercury on the side of the tube connected to the manometer is lower than before.
5) About 1.3 x 10-3 moles O2 were evolved.

Accepted Answer

A)  1, 2 and 5 only 
B)  5 only 
C)  2 and 4 only 
D)  3 and 4 only 
E)  4 and 5 only 
A)  1, 2 and 5 only 
B)  5 only 
C)  2 and 4 only 
D)  3 and 4 only 
E)  4 and 5 only

Question 19

The noxious gas H2S can be used to remove the acid rain component SO2 from factory emissions by the Claus Process. What volume of H2S in litres at STP will be needed to remove 2.00 kg of SO2?
2 H2S(g) + SO2(g)  $\rarr$ 3 S(s) + 2 H2O(l)

Accepted Answer

A)  1400 litres 
B)  7 litres 
C)  700 litres 
D)  350 litres 
E)  50 litres 
A)  1400 litres 
B)  7 litres 
C)  700 litres 
D)  350 litres 
E)  50 litres

Question 20

Do calculations involving water vapour pressure and relative humidity and describe some of the basic chemistry of the troposphere.

Accepted Answer

Water vapor pressure and relative humidi

The ideal gas equation is expected to be valid at

Consider the van der Waals "b" coefficient for He, O₂ andCO₂ increases because

A hair spray bottle will explode if under 9 atm of internal pressure. If this bottle is originally under 5 atm of pressure at 25˚C and is placed to close to a campfire and raises to 48˚C, what will be the pressure inside the bottle now?

If atmospheric pressure atop Mount Everest is about 250 mm Hg, what is the partial pressure of oxygen?

A gas mixture containing oxygen, nitrogen, and helium; if the partial pressure and mole fraction of oxygen is 425 Torr and 0.46, respectively, and the partial pressure of helium is 74 Torr, what is the partial pressure (in bar) of nitrogen in the mixture?

Consider a sample of gas in a tank. Under which of the following conditions would you expect the least ideal behaviour?

If the relative humidity at 28°C is 58.3 %, what is the dew point?

The level of mercury on the sample side of a manometer is 56 mm below that of the atmospheric side. If the atmospheric pressure is 1.05 bar, what is the pressure of the gas sample (in bar)?

A sample of gas is cooled to its vapourization temperature. What is true before the sample reaches equilibrium between the liquid and gaseous phases?

Consider the van der Waals "a" coefficient for He, O₂ andC₆H₆ increases because

Consider the van der Waals equation:

Which will occupy a larger volume, 10 moles of H₂(g) or 10 moles of propane, C₃H₈ (g)?

Cooling the gas in a container lowers the pressure because

If the compressibility factor, pV/nRT is 1 at pressure p, then

Methylamine, whose line structure is shown below, is one of the substances for the "fishy" odour of not-so-fresh fish. What is the average velocity and average kinetic energy (kJ/mole) of gaseous methylamine molecules at 25°C?

If 760 Torr is equivalent to 1 atm and to 1.01325 bar, then a pressure of 1 bar is equivalent to

The noxious gas H₂S can be used to remove the acid rain component SO₂ from factory emissions by the Claus Process. What volume of H₂Sin litres at STP will be needed to remove 2.00 kg of SO₂? 2 H₂S₍_g) + SO_2(g) $\rarr$ 3 S_(s) + 2 H₂O_(l)

Do calculations involving water vapour pressure and relative humidity and describe some of the basic chemistry of the troposphere.

Fundamental Concepts of Chemistry

Energy and Its Conservation

Atoms and Light

Atomic Energies and Periodicity

Fundamentals of Chemical Bonding

Theories of Chemical Bonding

Effects of Intermolecular Forces

Properties of Solutions

Organic Chemistrystructure

Organic Chemistryreactions

Spontaneity of Chemical Processes

Kinetics: Mechanisms and Rates of Reactions

Principles of Chemical Equilibrium

Aqueous Acidbase Equilibria

Applications of Aqueous Equilibria

Electron Transfer Reactions

Macromolecules

The Transition Metals

The Main Group Elements

Nuclear Chemistry and Radiochemistry

Filters

Exam 2: The Behaviour of Gases

The ideal gas equation is expected to be valid at

Consider the van der Waals "b" coefficient for He, O2 and CO2 increases because

A hair spray bottle will explode if under 9 atm of internal pressure. If this bottle is originally under 5 atm of pressure at 25˚C and is placed to close to a campfire and raises to 48˚C, what will be the pressure inside the bottle now?

If atmospheric pressure atop Mount Everest is about 250 mm Hg, what is the partial pressure of oxygen?

A gas mixture containing oxygen, nitrogen, and helium; if the partial pressure and mole fraction of oxygen is 425 Torr and 0.46, respectively, and the partial pressure of helium is 74 Torr, what is the partial pressure (in bar) of nitrogen in the mixture?

Consider a sample of gas in a tank. Under which of the following conditions would you expect the least ideal behaviour?

If the relative humidity at 28°C is 58.3 %, what is the dew point?

The level of mercury on the sample side of a manometer is 56 mm below that of the atmospheric side. If the atmospheric pressure is 1.05 bar, what is the pressure of the gas sample (in bar)?

A sample of gas is cooled to its vapourization temperature. What is true before the sample reaches equilibrium between the liquid and gaseous phases?

Consider the van der Waals "a" coefficient for He, O2 and C6H6 increases because

Consider the van der Waals equation:

Which will occupy a larger volume, 10 moles of H2 (g) or 10 moles of propane, C3H8 (g)?

Cooling the gas in a container lowers the pressure because

If the compressibility factor, pV/nRT is 1 at pressure p, then

Methylamine, whose line structure is shown below, is one of the substances for the "fishy" odour of not-so-fresh fish. What is the average velocity and average kinetic energy (kJ/mole) of gaseous methylamine molecules at 25°C?

If 760 Torr is equivalent to 1 atm and to 1.01325 bar, then a pressure of 1 bar is equivalent to

The noxious gas H2S can be used to remove the acid rain component SO2 from factory emissions by the Claus Process. What volume of H2S in litres at STP will be needed to remove 2.00 kg of SO2? 2 H2S(g) + SO2(g) →\rarr→ 3 S(s) + 2 H2O(l)

Do calculations involving water vapour pressure and relative humidity and describe some of the basic chemistry of the troposphere.

Fundamental Concepts of Chemistry

Energy and Its Conservation

Atoms and Light

Atomic Energies and Periodicity

Fundamentals of Chemical Bonding

Theories of Chemical Bonding

Effects of Intermolecular Forces

Properties of Solutions

Organic Chemistrystructure

Organic Chemistryreactions

Spontaneity of Chemical Processes

Kinetics: Mechanisms and Rates of Reactions

Principles of Chemical Equilibrium

Aqueous Acidbase Equilibria

Applications of Aqueous Equilibria

Electron Transfer Reactions

Macromolecules

The Transition Metals

The Main Group Elements

Nuclear Chemistry and Radiochemistry

Filters

Consider the van der Waals "b" coefficient for He, O₂ andCO₂ increases because

Consider the van der Waals "a" coefficient for He, O₂ andC₆H₆ increases because

Which will occupy a larger volume, 10 moles of H₂(g) or 10 moles of propane, C₃H₈ (g)?

The noxious gas H₂S can be used to remove the acid rain component SO₂ from factory emissions by the Claus Process. What volume of H₂Sin litres at STP will be needed to remove 2.00 kg of SO₂? 2 H₂S₍_g) + SO_2(g) $\rarr$ 3 S_(s) + 2 H₂O_(l)